The Gibbs energy for given reaction has to be calculated using given cell potential. 2 N A D H + O 2 + 2 H + → 2 N A D + + 2 H 2 O E c e l l = 1.14 V Concept Introduction: Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation. The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell. The relation between the cell potential E cell and the Gibbs energy is − ν F E c e l l = Δ r G h e r e , E c e l l − c e l l p o t e n t i a l Δ r G − G i b b s e n e r g y F − F a r a d a y ' s c o nstant ν − n o . o f e l e c t r o n s

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Answer 1

Question

Chapter 5, Problem 5.70P

(a)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

2NADH+O2+2H+→2NAD++2H2O Ecell=1.14 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

(b)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

Malate+NAD+→oxaloacetate + NADH + H+ Ecell=−0.154 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

(c)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

O2+4H++4e−→2 H2O Ecell=0.81V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

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Answer 2

Question

Chapter 5, Problem 5.70P

(a)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

2NADH+O2+2H+→2NAD++2H2O Ecell=1.14 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

(b)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

Malate+NAD+→oxaloacetate + NADH + H+ Ecell=−0.154 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

(c)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

O2+4H++4e−→2 H2O Ecell=0.81V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 5, Problem 5.70P

(a)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

2NADH+O2+2H+→2NAD++2H2O Ecell=1.14 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

(b)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

Malate+NAD+→oxaloacetate + NADH + H+ Ecell=−0.154 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

(c)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

O2+4H++4e−→2 H2O Ecell=0.81V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 5, Problem 5.70P

(a)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

2NADH+O2+2H+→2NAD++2H2O Ecell=1.14 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

(b)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

Malate+NAD+→oxaloacetate + NADH + H+ Ecell=−0.154 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

(c)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

O2+4H++4e−→2 H2O Ecell=0.81V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 5

Chapter 5, Problem 5.70P

(a)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

2NADH+O2+2H+→2NAD++2H2O Ecell=1.14 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

(b)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

Malate+NAD+→oxaloacetate + NADH + H+ Ecell=−0.154 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

(c)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

O2+4H++4e−→2 H2O Ecell=0.81V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

Answer 6

Chapter 5, Problem 5.70P

(a)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

2NADH+O2+2H+→2NAD++2H2O Ecell=1.14 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

Answer 7

Chapter 5, Problem 5.70P

(a)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

2NADH+O2+2H+→2NAD++2H2O Ecell=1.14 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

Answer 8

(b)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

Malate+NAD+→oxaloacetate + NADH + H+ Ecell=−0.154 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

Answer 9

(b)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

Malate+NAD+→oxaloacetate + NADH + H+ Ecell=−0.154 V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

Answer 10

(c)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

O2+4H++4e−→2 H2O Ecell=0.81V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

Answer 11

(c)

Interpretation Introduction

Interpretation:

The Gibbs energy for given reaction has to be calculated using given cell potential.

O2+4H++4e−→2 H2O Ecell=0.81V

Concept Introduction:

Electrochemical cells: Both oxidation and reduction occur at the same moment in an electrochemical cell. The oxidation process occurs at the anode while the reduction process occurs at the cathode in the cell. The concentration of the electrode (anode or cathode) in the half-cells and cell potential (voltage) can be calculated with the help of Nernst equation.

The production of electric current from spontaneous reaction occurring from the electrochemical cell is defined as galvanic cell.

The relation between the cell potential Ecell and the Gibbs energy is

−νFEcell=ΔrGhere, Ecell− cell potential ΔrG−Gibbs energy F−Faraday's constant ν− no. of electrons

Answer 12

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

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Answer 15

Ch. 5 - Prob. 5A.1ST Ch. 5 - Prob. 5A.2ST Ch. 5 - Prob. 5A.3ST Ch. 5 - Prob. 5A.4ST Ch. 5 - Prob. 5A.5ST Ch. 5 - Prob. 5B.1ST Ch. 5 - Prob. 5B.2ST Ch. 5 - Prob. 5B.3ST Ch. 5 - Prob. 5C.1ST Ch. 5 - Prob. 5C.2ST

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